Chapter #17 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. Are all liquids soluble in one another? Explain. Get solution

2. Gasoline is a nonpolar solvent; water is a polar solvent. Is KCl more likely to be soluble in gasoline or in water? Get solution

3. Compare the solubility of common table salt, NaCl, with that of naphthalene (moth flakes), C10H8, in (a) water, (b) gasoline. Get solution

4. How do a mixture, a solution, and a pure compound differ in composition? Get solution

5. Explain what “like dissolves like” means. Get solution

6. Give an example of solvation involving ion-dipole interaction. Get solution

7. A solution is made by dissolving sugar in water. Which is the solvent and which the solute? Get solution

8. Suppose a solution contains either stilt or sugar dissolved in water. Suggest a simple way by which you could easily tell which it is. Get solution

9. One mole of sugar is added to 1 liter of water. Is the concentration of the solution 1 M? Explain. Get solution

10. Calculate (a) the number of moles and (b) the number of grams of NaCl in 50.0 mL of 2.00 M NaCl. Get solution

11. Describe how you would prepare 250 mL of 0.100 M NaOH from solid NaOH and water. Get solution

12. A sample of rainwater has a nitric acid concentration of 3.00 × 10−8 M. How many grams of nitric acid are present in 1 liter? Get solution

13. Explain how you would make a 1.50-m calcium chloride solution. Get solution

14. How many grams of water would you have to add to 1000 g of sugar, C12H22O11, in order to prepare a 1-m solution? Get solution

15. How many molecules of ethyl alcohol, C2H5OH, must be dissolved in 500 g of water to make a 1-m solution? Get solution

16. An analysis of rainwater revealed a concentration of nitric acid, HNO3, of 2.2 × 10−6 g/liter. What is the molarity with respect to the nitric acid? Get solution

17. What is the meaning of the word “colligative” in the context of colligative properties? Get solution

18. Explain why seawater has a lower freezing point than fresh water. Get solution

19. How can you determine experimentally whether a substance is an electrolyte or a nonelectrolyte? Get solution

20. Which will freeze faster, a fresh-water pond or a salt-water pond? Get solution

21. How does the spreading of salt on ice-covered walks and roads cause the ice to melt? Get solution

22. Discuss the principle whereby the addition of antifreeze to an automobile radiator exerts its action. Get solution

23. The solution in a car radiator froze at 0°F. Determine the molality of the solution. Get solution

24. A solution contains 684 g of sucrose, C12H22O11, per 1000 g of water. Determine the freezing point of the solution. Get solution

25. A solution is made by dissolving 45.0 g of dextrose (C6H12O6) in 250.0 g of water.(a) Calculate the molality.(b) At what temperature will the solution freeze? Get solution

26. Which solution would produce the brighter light in an electrical conductivity apparatus, 0.100 M NaCl or 0.100 M Na3PO4? Explain. Get solution

27. List some general properties of acids. Get solution

28. List some general properties of bases. Get solution

29. In the Arrhenius definition, (a) what characterizes an acid; (b) what characterizes a base? Get solution

30. What does it mean to say that an acid is strong in aqueous solution? Get solution

31. When aqueous solutions of sodium chloride and silver nitrate are mixed, a precipitate forms instantaneously. How does the Arrhenius theory explain this result? Get solution

32. Complete and balance the following equations representing neutralization reactions:(a) HCl + Ca(OH)2 →(b) NH3 + H2SO4 →(c) NaOH + HNO3 →(d) H3PO4 + LiOH → Get solution

33. Why is the acidity of a solution expressed in terms of its pH rather than in terms of the molarity of hydrogen ion present? Get solution

34. How is pH defined? Get solution

35. Vinegar is an aqueous solution of acetic acid. Would you expect the pH of vinegar to be greater than or less than 7.00? Get solution

36. State whether each of the following solutions is acidic or basic. The H+ concentrations are given.(a) [H+] = 1.00 × 10−4 M(b) [H+] = 1.00 × 10−11 M(c) [H+] = 3.50 × 10−13 M(d) [H+] = 0.0001 M Get solution

37. Classify the following aqueous solutions as acidic, basic, or neutral if their pH is(a) 11. (b) 2. (c) 7. (d) 8.24. (e) 3.48. Get solution

38. Why can boric acid (H3BO3) be used in eyewashes, whereas hydrochloric acid (HCl) is not safe to use? Get solution

39. How do soaps and detergents cleanse? Get solution

40. In regions where the water supply is rich in calcium or magnesium compounds, why are detergents better cleaning agents than soaps? Get solution

41. Of what importance is biodegradability to the for-mulators of detergents? Get solution

42. What are the disadvantages of hard water? Get solution

43. What is the environmental impact of phosphorus compounds in detergents? Get solution

44. Why is an algal bloom—a thick mat of blue-green algae—on the surface of a lake an undesirable sign? Get solution

45. Plow can eutrophication lead to the death of a lake? Get solution

46. Multiple ChoiceA. Which of the following would be most soluble in the polar solvent water?(a) I2 (b) NaCl (c) CCl4 (d) N2B. The freezing point of H2o is(a) lowered by the addition of a solute.(b) raised by the addition of a solute.(c) not affected by the addition of a solute.(d) does not depend on the amount of solute added.C. When 1 mole of NaCl is dissolved in a kilogram of water, the concentration is(a) 0.50 molal.(b) 0.50 molar.(c) 1.00 molal.(d) 1.00 molar.D. A solution that has a pH of 7 is(a) slightly acidic.(b) strongly acidic.(c) neutral.(d) slightly basic.E. Kw(a) equals 10−14.(b) is the ion product of water.(c) equals [H3o+][OH-].(d) all of theseF. Which of the following is not a solution?(a) air free of smoke and dust(b) water free of other substances(c) sugar in water(d) HCl in waterG. When sodium chloride dissolves in water, the following species would be found in the resulting solution:(a) solvated NaCl molecules(b) solvated Na+(c) solvated Cl−(d) (b) and (c)H. Which one of the following observations is caused by a colligative property of solutions?(a) Water freezes at a lower temperature under pressure.(b) Water boils at a higher temperature under pressure.(c) Salt dissolves more rapidly in hot water than in cold.(d) Ice melts at a lower temperature when salt is added.I. A small amount of a certain solute melting at 800°C is added to water. The solution will be expected to freeze(a) above room temperature.(b) at 0°C.(c) slightly above 0°C.(d) slightly below 0°C.J. The pH of a solution refers to(a) the molarity of an acidic solution.(b) the molality of an acidic solution.(c) the concentration of hydronium ions in solution.(d) all of these. Get solution

Chapter #16 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. Discuss a method that might be used to measure the rate of a reaction. Get solution

2. Although a lump of coal burns slowly, a mine full of coal dust may explode. Explain. Get solution

3. Why do iron filings burn more rapidly in pure O2 than in air? Get solution

4. Why does a 10°C rise in temperature have a marked effect on the rate of many chemical reactions? Get solution

5. Milk quickly spoils if left at room temperature but keeps for several days in a refrigerator. Explain. Get solution

6. Why do reaction rates usually increase with increasing temperatures? Get solution

7. Discuss the collision model for chemical reactions. Get solution

8. Describe how a catalyst may accelerate a chemical reaction. Get solution

9. Biochemical reactions occur in our bodies at atmospheric pressure and at about 37°C. Explain why higher pressures and temperatures are usually required to carry out similar reactions in the laboratory. Get solution

10. Methane burns vigorously in oxygen, yet a mixture of methane and oxygen can be kept indefinitely without reacting. Explain. Get solution

11. If you wished a reaction to go faster, what might you try to accomplish this? Get solution

12. What is the role of activation energy in the rate of a reaction? Get solution

13. Equilibrium represents the balancing of opposing processes. Explain why a vapor pressure above a liquid in a closed container represents an equilibrium. Get solution

14. A chemical reaction may be reversible or irreversible. How would you classify burning a piece of paper? Get solution

15. A chemical equilibrium is indicated by writing two opposing arrows, .... Explain. Get solution

16. Explain why reactants are not converted completely to products in many chemical reactions. Get solution

17. What does it mean to say that a chemical equilibrium is a dynamic system? Get solution

18. Discuss the principle of dynamic equilibrium as it applies to the system.... Get solution

19. What does the equilibrium constant for a reaction represent? Get solution

20. What do square brackets [ ] indicate when we write an equilibrium constant? Get solution

21. If the reaction...is at equilibrium, are the concentrations of NO, O2, and NO2 necessarily equal? Get solution

22. Write expressions for tire equilibrium constants of the following reactions.(a) ...(b) ...(c) ... Get solution

23. For which of the following systems does the reaction go least to completion in the forward direction: (a) K = 10−10; (b) K = 1; (c) K = 104? Get solution

24. The rocket propellant hydrazine reacts with oxygen according to the following equation:...Write the equilibrium expression. Get solution

25. Sulfur dioxide contributes to atmospheric pollution through its oxidation to sulfur trioxide:...Determine the value of the equilibrium constant, K, for this reaction if the equilibrium concentrations of a mixture of the gases areSO2 = 4.20 × 10−7 mole/literSO3 = 0.500 mole/literO2 = 2.10 × 10−7 mole/liter Get solution

26. An equilibrium constant for a reaction is 3.20 × 107. Is the formation of products of reactants favored? Get solution

27. What does Le Châtelier’s principle tell us about maximizing the yield of a reaction? Get solution

28. What change in conditions changes the equilibrium constant K of a reaction? Get solution

29. For the equilibrium system...list four ways in which the concentration of SO3 at equilibrium could be increased. Get solution

30. For the reaction...what is the effect of (a) an addition of N2? (b) an increase in temperature? (c) an increase in pressure? Get solution

31. Will an increase in temperature cause the following equilibrium system to shift to the left, shift to the right, or have no effect?... Get solution

32. Predict the effect of (a) an increase in the concentration of one reactant; (b) an increase in pressure; (c) an increase in temperature; and (d) the introduction of a catalyst upon the following reactions at equilibrium:1. ...2. ... Get solution

33. Explain how increasing the temperature would affect the equilibrium... Get solution

34. Multiple ChoiceA. Which of the following would probably slow down the rate of a reaction?(a) increasing the temperature(b) increasing the concentration(c) using a larger beaker(d) lowering the temperatureB. The principal reason for the increase in reaction rate with temperature is(a) molecules collide more frequently.(b) the pressure increases.(c) the activation energy increases.(d) the fraction of high-energy molecules increases.C. Which of the following changes will increase the yield of products at equilibrium?(a) an increase in temperature(b) an increase in pressure(c) addition of a catalyst(d) increasing reactant concentrationsD. What is the effect of increasing the concentration of B in the reaction ...?(a) the value of K decreases(b) the value of K increases(c) the equilibrium shifts to the right(d) the equilibrium shifts to the leftE. A catalyst speeds up a reaction by(a) increasing the energy released.(b) decreasing the energy released.(c) increasing the activation energy.(d) decreasing the activation energy.F. To speed up a reaction, all of the following will work except(a) increasing the concentrations of the reactants.(b) adding a suitable catalyst.(c) lowering the temperature.(d) creating more surface area by pulverizing a solid reactant.G. Which one of the following changes has no effect on the position of equilibrium?(a) an increase in temperature(b) a decrease in temperature(c) addition of a catalyst(d) addition of a productH. When a reaction has reached equilibrium,(a) all reaction ceases.(b) the rate of the forward reaction becomes zero.(c) the concentrations of reactants and products are equal.(d) the rates of the forward and reverse reactions are equal.I. The value of K for a particular reaction changes if(a) the temperature is changed.(b) the concentration is changed.(c) a catalyst is added.(d) but K never changes.J. Chemical kinetics is the study of(a) equilibrium.(b) reaction rates.(c) catalysis.(d) solutions. Get solution

Chapter #15 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. What is the difference between an atom and an ion? Get solution

2. Give the symbol and oxidation number for each of the following ions.(a) aluminum ion(b) silver ion(c) oxide ion(d) copper(II) ion(e) ferric ion Get solution

3. What is a polyatomic ion? Get solution

4. Give the formula and charge for each of the following polyatomic ions.(a) sulfate ion(b) chlorite ion(c) phosphate ion(d) nitrite ion(e) hydroxide ion Get solution

5. What does a chemical formula represent? Get solution

6. How does the principle of electroneutrality apply to a chemical formula? Get solution

7. Write the formulas of the following binary ionic compounds.(a) calcium oxide(b) potassium iodide(c) zinc chloride(d) aluminum sulfide(e) sodium phosphide Get solution

8. Write the formulas of the following binary ionic compounds.(a) copper(I) oxide(b) lead(II) chloride(c) tin(II) fluorided) iron(III) sulfide(e) nickel(II) bromide Get solution

9. Write the formulas of the following compounds.(a) stannic fluoride(b) cuprous oxide(c) ferrous sulfide(d) plumbic iodide(e) cobaltous phosphide Get solution

10. Write the formulas of the following ternary ionic compounds.(a) barium sulfate(b) lead(IV) chromate(c) stannic carbonate(d) ferrous nitrate(e) tin(II) acetate Get solution

11. Give the traditional name (using -ous or -ic to indicate the charge of the cat ion) of each of the following binary ionic compounds.(a) Fe2S3(b) HgCl2(c) SnI4(d) CuBr2(e) PbO Get solution

12. Give the Stock name (using a Roman numeral to specify the charge of the cation) for each of the following binary ionic compounds.(a) PbI4(b) SnO(c) CuS(d) Fe2S3(e) AuCl3 Get solution

13. Name each of the following ternary ionic compounds, giving both the traditional and the Stock names.(a) FePO4(b) CuSO4(c) Sn(NO2)2(d) Pb(CrO4)2(e) Au(ClO)3 Get solution

14. Determine the molar mass of C7H5N3O6 (TNT). Get solution

15. What is the percent composition of cholesterol, C22H45OH? Get solution

16. An insecticide, parathion, has the formula C2H14PNSO5. What is its percent composition? Get solution

17. Determine the percentage of iodine in thyroxine, C14H11O4NI4, a compound produced in the th yroid gland. Get solution

18. Tetraethyl lead, Pb(C2H5)4, was widely used as an additive in gasoline to increase the octane rating. Determine the percentage of lead present. Get solution

19. Which of the following compounds contains the highest percentage of nitrogen?(a) KNO3(b) NCl3(c) CO(NH2)2(d) Fe(CN)2 Get solution

20. What does the mole have in common with the pair or the dozen? Get solution

21. (a) Why isn’t the dozen used for counting atoms?(b) Why isn’t the mole used for counting eggs? Get solution

22. What is the mass of one atom of platinum? Get solution

23. How many atoms are present in 1 kilogram of silver? Get solution

24. What is the mass of one molecule of sucrose, C12H22O11? Get solution

25. How many grams of vitamin C, C6H8O6, are there in 0.731 mol of vitamin C? Get solution

26. What is the mass in grams of a molecule of hemoglobin if the molar mass is about 68,000? Get solution

27. What information about a new compound must be known before its formula can be determined? Get solution

28. What does the empirical formula of a compound represent? Get solution

29. Give the empirical formula of each of the following compounds.(a) C4H10(b) N2O4(c) B2H6(d) Na2S2O4(e) K2Cr2O7 Get solution

30. The empirical formula of dextrose is CH2O, and the molar mass is 180. What is the molecular formula of dextrose? Get solution

31. The empirical formula of butane is C2H5. If the molar mass of butane is 58, what is its molecular formula? Get solution

32. Ethyl alcohol shows the following analysis: 52.2% C, 13.0% H, 34.8% O. What is its molecular formula if it has a molar mass of 46? Get solution

33. Urea shows the analysis 20.0% C, 6.7% H, 46.7% N, 26.6% O. What is its empirical formula? Get solution

34. What is the molecular formula of aspirin if its molar mass is 180.2 and analysis shows 60.0% C, 4.48% H, and 35.5% O? Get solution

35. What is the difference between a chemical reaction and a chemical equation? Get solution

36. Sodium forms an ionic compound with sulfur.(a) Give the chemical formula of the compound.(b) Name the compound.(c) Write a balanced equation for the reaction. Get solution

37. Aluminum cans react with oxygen to form aluminum oxide. Write the balanced equation for this reaction. Get solution

38. The following reaction represents the combustion of a hydrocarbon (octane):C8H18 + O2 → CO2 + H2OBalance the equation. Get solution

39. Iron rust forms when iron reacts with oxygen to form iron(III) oxide. Write the balanced equation for this reaction. Get solution

40. Excess carbon dioxide is removed from the atmosphere of a spacecraft by lithium hydroxide. The products are lithium carbonate and water. Write a balanced equation for this reaction. Get solution

41. Aluminum sulfate reacts with calcium hydroxide to form a gelatinous compound, aluminum hydroxide, and calcium sulfate. Suspended solids in water-supply systems are removed by the aluminum hydroxide and settle to the bottom. Write a balanced equation for the reaction. Get solution

42. Balance the following equations.(a) P + O2 → P4O10(b) Al + O2 → Al2O3(c) SO2 + O2 → SO3(d) NH3 → N2 + H2(e) H2O2 → H2O + O2(f) NH4NO3 → N2O + H2O(g) Zn + H3PO4 → Zn3 (PO4)2 + H2(h) Al + H2SO4 → Al2(SO4)3 + H2(i) NaNO3 + H2SO4 →(j) FeCl3 + H3PO4 → Get solution

43. Multiple ChoiceA. When silicon reacts with chlorine, the compound is(a) SiCl.(b) SiCl2.(c) SiCl3.(d) SiCl4.B. The formula for lead(II) sulfide is(a) PbS.(b) PbS2.(c) Pb2S.(d) Pb4S.C. The name of the compound CuSo4 is(a) copper sulfate.(b) cuprous sulfate.(c) copper(I) sulfate.(d) copper(II) sulfate.D. A mole of sodium chloride contains(a) 6.02 × 1023 ions.(b) 6.02 × 1023 molecules.(c) 1.20 × 1024 ions.(d) 1.20 × 1024 chloride ions.E. The numbers needed to balance the equation Al + F2 → AlF3 are(a) 1, 3, 2.(b) 2, 1, 2.(c) 4, 3, 2.(d) 2, 3, 2.F. The term “mole” refers to(a) the number of particles in an atom of an element.(b) the number 6.02 × 1023.(c) the number of atoms in a molecule.(d) the number of electrons in an atom of carbon.G. One mole of H2O molecules contains(a) 3.01 × 1023 molecules.(b) 6.02 × 1023 atoms.(c) 6.02 × 1023 hydrogen atoms.(d) 1.80 × 1024 atoms.H. An empirical formula indicates(a) the relative number of atoms in a molecule.(b) the three-dimensional structure of a molecule.(c) the molar mass of a molecule.(d) how atoms are bonded to one another in a moleculeI. The molecular formula for a gas that has an empirical formula CH and a molecular weight of 78 is(a) C5H2O.(b) C6H6.(c) C3H3.(d) C9H9.J. The name of the compound Mg3N2 is(a) manganese nitride.(b) magnesium nitride.(c) magnesium nitrite.(d) magnesium nitrate. Get solution

Chapter #14 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. List the noble gas elements. Get solution

2. What is the relation between the octet rule and a noble gas structure? Get solution

3. Explain why the chemical activity of tire noble gases went undiscovered for so long. Get solution

4. Draw the Lewis dot structures for the following atoms(a) N(b) Na(c) Cl(d) Ne(e) Br Get solution

5. The following substances are isoelectronic with one another. Write a Lewis structure for each.(a) CH4(b) NH3(c) H2O(d) HF(e) Ne Get solution

6. Write Lewis structures for the following compounds.(a) sodium fluoride: NaF(b) carbon tetrachloride: CCl4(c) boron trifluoride: BF3(d) molecular nitrogen: N2(e) carbon monoxide: CO Get solution

7. Differentiate between the molecular formula and Lewis formula of water. Get solution

8. Give the total number of outer-shell electrons in each of the following.(a) NH3(b) CaCl2(c) Al2S3(d) ...(e) ... Get solution

9. Write the Lewis structure for O2. What kind of bond has to be formed between the two oxygens to satisfy the octet rule? Get solution

10. Give the number of the periodic group and the number of valence electrons for each of the following atoms.(a) S(b) C(c) Mg(d) Ne(e) B Get solution

11. Does the Ca2+ ion possess a noble gas configuration? Explain. Get solution

12. Is the formula MgF3 likely to represent a stable compound? Explain. Get solution

13. Using Lewis structures, diagram the reaction that occurs between Ca atoms and F atoms. Get solution

14. Account for the fact that the second ionization energy of lithium (75.6 eV) is greater dian the first (5.4 eV). Get solution

15. (a) List four ions that are isoelectronic with the noble gas xenon, and (b) give the charge of each. Get solution

16. Write Lewis symbols to represent the electron transfer between K and S to form ions with noble gas configurations. Get solution

17. Explain why argon does not form ionic bonds. Get solution

18. What are the charges on the ions in Al2S3? Get solution

19. Why would it be misleading to refer to “molecules” of sodium chloride (NaCl) in the crystalline state? Get solution

20. Explain why the halogens (fluorine, chlorine, bromine, and iodine) occur as diatomic molecules. Get solution

21. How do a bromine atom, a bromine molecule, and a bromide ion differ? Write the formula for each. Get solution

22. Why does neon not form covalent bonds? Get solution

23. What is (a) a double bond; (b) a triple bond? Get solution

24. How many covalent bonds are normally formed by(a) F?(b) O?(c) N?(d) C? Get solution

25. Which electron pairs in tire Lewis formula of H2S are bonding and which are lone pairs? Get solution

26. How does a coordinate covalent bond differ from an ordinary covalent bond? Get solution

27. Predict (a) whether the bonds between the following pairs of elements would be ionic or covalent, and (b) if covalent, tire percent ionic character of tire bond.(a) Ba, O(b) Al, S(c) N, Cl(d) C, S(e) Si, C Get solution

28. Although fluorine is the most electronegative element, silicon tetrafluoride (SiF4) does not have-a dipole moment. Explain. Get solution

29. Based on the electronegativities of the atoms, arrange the following bonds in order of increasing ionic character.... Get solution

30. Why is an HCl molecule polar whereas a Cl2 molecule is nonpolar? Get solution

31. Predict whether a bond will form and, if so, whether it will be ionic or covalent, between(a) Br and F.(b) Li and Na.(c) K and S.(d) N and Ne. Get solution

32. Which atom in ClF is more negatively charged? Get solution

33. How do the electronegativities of the elements vary from (a) left to right across a period and (b) from the top to the bottom of a group? Get solution

34. What geometric structure would you predict for each of tire following substances?(a) CF4(b) BeCl2(c) BBr3(d) AsH3(e) SF6 Get solution

35. (a) What bond angle would you predict when all of the valence electrons of an atom are involved in three single bonds? (b) Would the presence of a lone pair of electrons in addition to three bonds change your prediction? If so, how? Get solution

36. On the basis of molecular structure, explain why NH3 has a dipole moment but BF3 does not. Get solution

37. The H2S molecule has a geometry similar to that of water. Is the H2S molecule a dipole? If so, where are the partial charges located? Get solution

38. How many atoms are directly bonded to the central atom in a tetrahedral molecule? Get solution

39. What are some properties of water that are determined by the presence of a dipole moment? Get solution

40. Explain why copper wire is a good conductor of electricity. Get solution

41. (a) List three types of solids based on the nature of the bonding forces, and (b) give an example of each. Get solution

42. Account for the characteristic luster of silver metal. Get solution

43. Why are metals good conductors of heat and electricity? Get solution

44. Account for the relatively high density of metals. Get solution

45. How are the atoms in a metal held together? Get solution

46. Multiple ChoiceA. In the Lews structure for fluorine, the number of dots surrounding the symbol for fluorine is(a) one.(b) four.(c) five.(d) seven.B. The most electronegative element on the Pauling electronegativity scale is(a) oxygen.(b) neon.(c) fluorine.(d) cesium.C. The kind of bonding in sodium chloride is(a) ionic.(b) covalent.(c) coordinate covalent.(d) metallic.D. The compound that has the greatest covalent character is(a) H2O.(b) NaCl.(c) Br2.(d) Fe2O3.E. The bond between two nitrogen atoms in nitrogen gas is(a) single.(b) double.(c) triple.(d) electrovalent.F. The chemical formula for the compound formed when 14Si reacts with 17Cl is(a) SiCl.(b) SiCl2.(c) SiCl3.(d) SiCl4.G. Which of the following molecules could not possibly be polar?(a) H2O(b) HCl(c) I2(d) NH3H. Sodium chloride has(a) ionic bonds.(b) covalent bonds.(c) nonpolar bonds.(d) coordinate covalent bonds.I. When K and O react to form the ionic compound K2O,(a) each potassium atom loses one electron.(b) each potassium atom loses two electrons.(c) each oxygen atom loses one electron.(d) each oxygen atom loses two electrons.J. A covalent bond is formed(a) when electrons are transferred.(b) when electrons are shared.(c) when a cation and anion come together.(d) only when shared electrons come from the same atom. Get solution

Chapter #13 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. Give the name of the element for each atomic symbol.(a) Pb(b) Sn(c) Hg(d) Ag(e) Si Get solution

2. Give the atomic symbol for each of the following elements.(a) potassium(b) sodium(c) phosphorus(d) aluminum(e) fluorine Get solution

3. Give the symbols and names of the elements whose symbols consist of only one letter. Get solution

4. Name five elements whose symbols appear to be unrelated to the names we use for the elements. Get solution

5. Give the number of electrons, protons, and neutrons for these environmentally important elements: (a) fluorine-19; (b) sulfur-32; (c) arsenic-75; (d) strontium-88; (e) mercury-201. Get solution

6. Determine the nuclear structure of the following isotopes: (a) ...; (b) ...; (c) .... Get solution

7. The abundances of the isotopes of magnesium (based on the mass of 12C as 12.00000) are as follows:...Determine the atomic mass of magnesium. Get solution

8. When Mt. St. Helens erupted in 1980, a considerable amount of a radioactive element was produced. The atomic number of the element is 86. What are the name, symbol, and atomic mass of this element? Get solution

9. Give the mass of an atom with(a) 49 protons, 49 electrons, 64 neutrons.(b) 31 protons, 31 electrons, 38 neutrons.(c) 91 protons, 91 electrons, 140 neutrons. Get solution

10. Determine the number of neutrons in each of the following.(a) a nitrogen atom of mass number 13(b) a potassium atom of mass number 41(c) a lead atom of mass number 207 Get solution

11. Where in the atom are these particles located?(a) protons(b) electrons(c) neutrons Get solution

12. How many nucleons are there in each of the following?(a) 40Ca(b) 56Fe(c) zinc-65(d) iodine-127 Get solution

13. Which of the following atoms are isotopes of each other?(a) ...(b) ...(c) ... Get solution

14. Do the symbols ... and ... have the same meaning? Explain. Get solution

15. Cobalt-60 is used in radiation therapy for certain cancers. How many(a) protons are in its nucleus?(b) neutrons are in its nucleus?(c) electrons are in a cobalt atom? Get solution

16. In what way do the isotopes copper-63 and copper-65 differ from each other? Get solution

17. Are there any atoms that have no neutrons? Explain. Get solution

18. Arrange the following in order of increasing mass.(a) 2 Na atoms(b) 3 Mg atoms(c) a K atom Get solution

19. Name the elements associated with the following electron configurations.(a) 1s22s2(b) [Ne] 3s1(c) [Ar] 4s23d7(d) 1s22s22p63s23p64s23d104p5(e) [Kr] 5s24d105p2 Get solution

20. What experimental evidence is there for the idea that electronic spin is “quantized” in two possible directions? Get solution

21. In the energy level n = 3,(a) how many orbitals are possible?(b) what is the electron capacity of this level? Get solution

22. Write the electron configurations for (a) 5B; (b) 9F; (c) 21Sc; (d) 33As; (e) 56Ba. Get solution

23. The highest-energy electron of a chlorine atom is designated 3p5. (a) Explain why. (b) Deduce from this notation the values of the four quantum numbers (n, l, m, s). Get solution

24. (a) Construct an “electron-in-the-box” energy-level diagram for phosphorus, 15P. (b) What principle dictates the arrangement of the outermost electrons? Get solution

25. Relate the Heisenberg uncertainty principle to the idea of an electron orbital. Get solution

26. Explain why the following is not a possible set of quantum numbers for an electron in an atom: n = 2, l = 2, m = 0. Get solution

27. How many electrons in an atom can have the following sets of quantum numbers?(a) n = 2(b) n = 2, l = 0(c) n = 2, l = 0, m = 0 Get solution

28. Emission spectra can be used to confirm the presence of an element in a material. How is this possible? Get solution

29. On the basis of one property that you select, discuss the meaning of the term “periodic” in the expression “periodic table.” Get solution

30. Experiments are under way to synthesize element 114. In which group of the periodic table would you expect it to be located? Get solution

31. Sodium initiates the third period, and argon closes it. What feature of atomic structure do the elements in this period share? Get solution

32. What similarity in electronic arrangement is shared by the members of the nitrogen family? Get solution

33. Which of the following elements have fairly similar properties: Ne, Sr, Kr, Br, Rb, Ca, He, Cl, F, Li, K? Get solution

34. Why does the periodic table work? Get solution

35. Multiple ChoiceA. When the electron of a hydrogen atom is in the energy level n = 2, we say that(a) it emits light.(b) it is in the ground state.(c) it is in an excited state.(d) it ionizes the atom.B. The atomic number of gold is 79 and the mass number of one of its isotopes is 197. The number of neutrons is(a) 79.(b) 197.(c) 118.(d) 158.C. Elements in the same group in the periodic table(a) have similar chemical properties.(b) are called isotopes.(c) have consecutive atomic numbers.(d) make up a period of elements.D. The principle that a maximum of two electrons is allowed in any orbital is known as(a) Bohr’s Aufbau principle.(b) Heisenberg’s uncertainty principle.(c) Hund’s rule.(d) the Pauli exclusion principle.E. The total electron capacity of the energy level n = 4 is(a) 8.(b) 16.(c) 18.(d) 32.F. All of the following are located in the nucleus of atoms, except(a) protons.(b) electrons.(c) neutrons.(d) nucleons.G. An element has eight protons and seven neutrons. The element is(a) phosphorus.(b) nitrogen.(c) oxygen.(d) chlorine.H. Neutral atoms of 117Sn and 119Sn differ in(a) the number of protons in the nucleus.(b) the number of neutrons in the nucleus.(c) their atomic numbers.(d) the number of extranuclear electrons.I. The atomic weight of potassium is 39.1. We can conclude that(a) an atom of potassium has a mass of 39.1 g.(b) potassium is a mixture of different masses, the average of which is 39.1 u.(c) every atom of potassium has a mass of 39.1 u.(d) potassium is an isotope of 39Y.J. Experimental support for the arrangement of electrons in distinct energy levels is based primarily on(a) scattering experiments.(b) the photoelectric effect.(c) atomic spectra.(d) radioactivity. Get solution

Chapter #12 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. Discuss the basis for a claim that there is gold on the sun. Get solution

2. Calculate the wavelength of the second line of the Balmer series for hydrogen. Get solution

3. Calculate the wavelength of the third line of the Paschen series for hydrogen. Get solution

4. A photon is emitted from a hydrogen atom that undergoes a transition from the n = 4 state to the n = 2 state. Calculate the wavelength of the emitted photon. Get solution

5. Why does the “fingerprint” of an atom have more than one characteristic frequency of light? Get solution

6. Why was the Balmer series detected before the Lyman series? Get solution

7. Does a neon sign emit light of a continuous spectrum or only a few discrete wavelengths? Explain. Get solution

8. What do the lines in the spectrum of an atom represent? Get solution

9. How did Bohr’s model of the atom account for the Balmer and other spectral series of the hydrogen atom? Get solution

10. Compare radioactivity and X-rays. Get solution

11. What was the experimental basis of Rutherford’s concept of a nuclear atom? Get solution

12. Although hydrogen has but a single electron, the complete hydrogen spectrum consists of numerous lines. How do you account for this? Get solution

13. Discuss two instances in which classical electromagnetic theory failed to account for the experimental observations. Get solution

14. In what way are quanta of radiation a return to the corpuscular theory of light? Get solution

15. In the photoelectric effect, the energy of a photoelectron is less than that of the incident photon. Explain. Get solution

16. Yellow light can induce the photoelectric effect in a certain metal, but orange fight cannot. Would blue fight? Explain. Get solution

17. The human eye is most sensitive to light of approximately 5500 Å in wavelength. What is the energy in joules of such a photon? Get solution

18. Which photon has the greater energy—infrared or ultraviolet? Get solution

19. How does the frequency of an X-ray photon that is scattered by an electron compare with the frequency of the incident photon? Get solution

20. If the frequency of a photon is doubled, how is its energy affected? Get solution

21. If the wavelength of a photon is doubled, what happens to its energy? Get solution

22. Explain why ultraviolet light causes sunburn, but visible light does not. Get solution

23. Which colors of the visible spectrum have photons of higher energy? Get solution

24. Why was the Compton effect considered important for verifying Einstein’s idea of light quanta? Get solution

25. How did de Broglie’s hypothesis help to explain the stability of the atom? Get solution

26. What is the de Broglie wavelength of a 0.500-kilo-gram football traveling at 15.0 m/s? Get solution

27. Calculate the de Broglie wavelength associated with the earth, if its mass is 6.00 × 1024 kilograms and it revolves around the sun with a velocity of 3.00 × 104 m/s. Get solution

28. How is the wave-particle duality related to the concept of symmetry in nature? Get solution

29. Discuss the meaning of the dual nature of radiation and matter. Get solution

30. Account for the considerably greater detail seen in a bacterial specimen revealed by an electron microscope as compared with the same specimen revealed by a light microscope. Get solution

31. Is light a wave or a particle? Explain. Get solution

32. Is an electron a particle or a wave? Explain. Get solution

33. Calculate the momentum of a photon of wavelength 5000 Å. Get solution

34. Calculate the de Broglie wavelength in meters for a proton moving with a speed of 106 m/s. Get solution

35. What is the de Broglie wavelength in meters of a 75-kg person who is jogging at 5 m/s? Get solution

36. If matter has a wave nature, why is this not observable in our daily experiences? Get solution

37. Multiple ChoiceA. When light shines on a metal surface, the energy of the photoelectrons depends on the(a) intensity of the light.(b) frequency of the light.(c) velocity of the light.(d) all of these.B. A bright-line spectrum of an element(a) is concentrated at the red end.(b) is evenly distributed.(c) is concentrated at the blue end.(d) is characteristic of the element.C. Radioactivity is a property of(a) excited electrons.(b) ultraviolet light.(c) atomic nuclei.(d) X-rays.D. The quantum theory does not explain(a) interference.(b) the photoelectric effect.(c) the Compton effect.(d) line spectra.E. Compared with a light microscope, an electron microscope(a) uses less energy.(b) works faster.(c) can magnify in greater detail.(d) uses longer wavelengths.F. Energy equals Planck’s constant times(a) ....(b) mc.(c) mc2.(d) cλ.G. Rutherford’s gold-foil experiment was instrumental in establishing the concept of(a) an atom.(b) a molecule.(c) subatomic particles.(d) a nucleus in an atom.H. An alpha particle is(a) negatively charged.(b) electrically neutral.(c) a helium nucleus.(d) approximately the same as an electron.I. Experimental support for the arrangement of electrons in distinct energy levels is based primarily on(a) atomic spectra.(b) scattering experiments.(c) the photoelectric effect.(d) radioactivity.J. Which of the following forms of electromagnetic radiation is the most energetic?(a) red(b) ultraviolet(c) infrared(d) green Get solution

Chapter #11 Solutions - Physical Science with Modern Applications - Melvin Merken - 5th Edition

 

1. If a positively charged glass rod attracts a pith ball suspended by a silk thread, must the pith ball be negatively charged? Explain. Get solution

2. Although rubbing a ball-point pen with a piece of flannel is not essential for electrifying the pen, it acquires a stronger charge than when it is merely in contact with the flannel. Explain. Get solution

3. Why is repulsion rather than attraction a conclusive test of electrification? Get solution

4. An unknown charge is brought near the knob of a positively charged electroscope, and the leaves converge. What is the nature of the unknown charge? Get solution

5. Assuming that an object is charged, explain how you would decide whether the charge is positive or negative. Get solution

6. Why is it more difficult to maintain an electric charge on an electroscope on a damp day than on a dry day? Get solution

7. Explain how you would charge an electroscope negatively by induction. Get solution

8. Explain how a charged body attracts an uncharged one. Get solution

9. Why do small bits of dry paper that are attracted to a charged comb often fly away when they touch the comb? Get solution

10. Explain why you may receive a shock from a metal door handle when you slide across a seat in an automobile. Get solution

11. The atoms of conductors and insulators are composed of the same constituents: electrons, protons, and neutrons. In what way, then, do conductors and insulators differ? Get solution

12. Name (a) three good conductors of electricity, and (b) three good insulators. Get solution

13. (a) In what ways are electrical forces and gravitational forces similar? (b) In what ways do they differ? Get solution

14. In hydrogen, the simplest atom, the electron and the proton (nucleus) are separated by 0.530 angstrom unit. If the charge on each is 1.60 × 10−19 coulomb (–for the electron, + for the proton), what is the force between them? Get solution

15. Calculate the force between two electrons that are separated by 10−9 meter. (Charge on the electron is − 1.60 × 10−19 coulomb.) Get solution

16. Explain the discharge of a lightning stroke between a negatively charged cloud and the earth. Get solution

17. How does an automobile that has a metal top and body shield its occupants from lightning? Get solution

18. Why is standing in an open field during a thunderstorm a dangerous practice? Get solution

19. (a) In what ways are electric charges and magnetic poles similar? (b) Different? Get solution

20. Why may heating reduce the strength of a magnet? Get solution

21. Discuss the significance of Faraday’s and Henry’s discovery of the production of an electric current by means of magnetism. Get solution

22. Can you create monopoles by breaking a bar magnet in half? Explain. Get solution

23. Like poles repel, yet the north-seeking pole of a magnet is attracted to the geographic North Pole of the earth. Explain. Get solution

24. Explain why a nail is attracted to either pole of a magnet, but another magnet is attracted to only one of the poles. Get solution

25. A magnet can be weakened by dropping it on a hard floor. Explain. Get solution

26. The atoms in a piece of wood are tiny magnets, yet the piece of wood is not. Explain. Get solution

27. Why will an unmagnetized nail that is in contact with a magnet attract an unmagnetized paper clip? Get solution

28. Discuss the meaning of the term “electric field.” Get solution

29. Calculate the magnitude and direction of the electric field 3.00 meters from a positive charge of 10−5 coulomb. Get solution

30. Sketch the electric field pattern between two point charges of opposite sign separated by a small distance. Get solution

31. (a) Two bar magnets are placed with their south poles facing each other. Represent the magnetic field between them in a diagram.(b) Repeat with the north pole of one magnet opposite the south pole of the second magnet. Get solution

32. A transistor radio draws 0.500 ampere of current. If it uses a 9.00-volt battery, what is the resistance of the radio? Get solution

33. What is the current through a 60.0-watt lamp that operates at 120 volts? Get solution

34. How many electrons flow through the filament of a 120-volt, 60.0-watt light bulb per second? Get solution

35. When people say that they left lights in the house “burning,” is this a correct statement? How might it have originated? Get solution

36. An electric clock uses 5.00 milliamperes of current on 120 volts. Find its resistance. Get solution

37. Why is it dangerous to replace a 15-ampere fuse that blows repeatedly with one having a larger current rating? Get solution

38. How much current flows through a 60.0-watt headlight of an automobile that has a 12-volt electrical system? Get solution

39. Calculate the resistance of a vacuum cleaner that uses a current of 14.0 amperes and operates on 120 volts. Get solution

40. Three incandescent lamps with resistances of 220, 440, and 660 ohms are connected in parallel across a 110-volt fine.(a) What is their combined resistance?(b) What total current is drawn by the three lamps?(c) How much current does each lamp draw? Get solution

41. Explain why operating too many electrical devices at one time may cause a fuse to blow. Get solution

42. Are the currents in resistors that are connected in parallel generally the same? Explain. Get solution

43. (a) What is the total resistance of five 20-ohm resistors connected in series? (b) Parallel? Get solution

44. Three resistors of 5, 10, and 15 ohms each are connected in series in a circuit with a 9.0-volt battery. What is the current through each resistor? Get solution

45. A 100-watt lamp draws 0.800 ampere in operation. What is its resistance? Get solution

46. Which uses more energy: a 250-watt TV set in 1 hour or a 1200-watt toaster in 10 minutes? Get solution

47. A 100-watt lamp was accidentally left burning in a storeroom for one week. How much did it cost at 10 cents per kilowatt-hour? Get solution

48. An electric range draws 20 amperes at 240 volts. What does it cost per hour to operate at 10 cents per kilowatt-hour? Get solution

49. Does a 5000-watt heater use twice the energy of a 2500-watt heater? Explain. Get solution

50. Multiple ChoiceA. The force of attraction between two charged spheres can be calculated from(a) Newton's second law.(b) Coulomb’s law.(c) Joule’s law.(d) Ohm’s law.B. An instrument for determining the magnitude of a charge is the(a) Van de Graaff generator.(b) electrostatic precipitator.(c) electroscope.(d) electrophorus.C. An electric current in a wire is a flow of(a) atoms.(b) protons.(c) ions.(d) electrons.D. Regions where the magnetic fields of atoms are fined up in the same direction are known as(a) superconductors.(b) magnetic domains.(c) currents of spinning electrons.(d) dynamos.E. A magnetic field is produced by(a) static negative charges.(b) an electron current.(c) static positive charges.(d) falling water.F. Which of the following substances differs from the others with respect to electricity?(a) plastic(b) glass(c) copper(d) cottonG. A natural magnet is(a) iron.(b) amber.(c) aluminum.(d) lodestone.H. Ohm’s law is correctly expressed by(a) ...(b) ...(c) R = VI.(d) I = VR.I. A fight bulb glows because(a) there is burning inside.(b) an electric current glows.(c) the filament is hot.(d) a very small current is flowing.J. Which of the following does not produce a magnetic field?(a) a current-carrying wire(b) a stationary electric charge(c) a moving electric charge(d) an electromagnet Get solution